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1

AIPMT 2015 Cancelled Paper

MCQ (Single Correct Answer)
If the value of equilibrium constant for a particular reaction is 1.6 $$ \times $$ 1012, then at equilibrium the system will contain
A
mostly products
B
similar amounts of reactants and products
C
all reactants
D
mostly reactants.

Explanation

As, 1.6 × 1012 is very high value of K. Thus, the reaction proceeds almost to completion and mixture must contain mostly products.
2

AIPMT 2015 Cancelled Paper

MCQ (Single Correct Answer)
Which of the following statements is correct for a reversible process in a state of equilibrium?
A
$$\Delta $$Go = $$-$$2.30 RT log K
B
$$\Delta $$Go = 2.30 RT log K
C
$$\Delta $$G = $$-$$2.30 RT log K
D
$$\Delta $$G = 2.30 RT log K

Explanation

$$\Delta $$G = $$\Delta $$Go + 2.303 RT log Q

At equilibrium, when $$\Delta $$G = 0 and Q = K

then 0 = $$\Delta $$Go + 2.303 RT log K

$$\Delta $$Go = – 2.303 RT log K
3

AIPMT 2015 Cancelled Paper

MCQ (Single Correct Answer)
The Ksp of Ag2CrO4,  AgCl,  AgBr  and Agl  are respectively, 1.1 $$ \times $$ 10$$-$$12, 1.8 $$ \times $$ 10$$-$$10, 5.0 $$ \times $$ 10$$-$$13, 8.3 $$ \times $$ 10$$-$$17. Which one of the following salts will precipitate last if AgNO3 solution is added to the solution containing equal moles of NaCl, NaBr, Nal and Na2CrO4?
A
AgBr
B
Ag2CrO4
C
Agl
D
AgCl

Explanation

From the Ksp values of the given salts calculate the solubility values. Salt having highest solubility will precipitate at last.
AgCrO4 2Ag+ + CrO42-
s 2s s


Ksp = (2s)2(s) = 1.1 × 10–12

$$ \Rightarrow $$ s = 0.65 × 10–4

AgCl Ag+ + Cl-
s s s


Ksp = s × s

$$ \Rightarrow $$ 1.8 × 10–10 = s 2

$$ \Rightarrow $$ s = 1.34 × 10–5

AgBr Ag+ + Br-
s s s


Ksp = s × s

$$ \Rightarrow $$ 5 × 10–13 = s2

$$ \Rightarrow $$ s = 0.71 × 10–6

AgI Ag+ + I-
s s s


Ksp = s × s

$$ \Rightarrow $$ 8.3 × 10–17 = s2

$$ \Rightarrow $$ s = 0.9 × 10–8

$$ \therefore $$ Solubility of Ag2CrO4 is maximum so, it will precipitate at last.
4

AIPMT 2015

MCQ (Single Correct Answer)
Which one of the following pairs of solution is not an acidic buffer ?
A
CH3COOH and CH3COONa
B
H2CO3 and Na2CO3
C
H3PO4 and Na3PO4
D
HClO4 and NaClO4

Explanation

An acidic buffer is a mixture of a weak acid and its salt with a strong base. Among CH3COOH, H2CO3, H3PO4 and HClO4, the HClO4 is a strong acid while all other are weak acid thus, HClO4 and NaClO4 does not constitute to form an acidic buffer.

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